The Final Exam

The CH141 exam will be on Monday, 12/17 at 1:30 -4:30 PM.   We will use the same Keyes first floor classrooms for the exam.   You may work for the entire 3 hours, but the exam is expected to take most students 120 min.  The exam will cover all class and laboratory materials and we will use the same format as the hour exams.   Allowed exam items are pens/pencils and a course-approved calculator. You will be provided with a periodic table and equation sheet.   You may bring snacks and a water bottle.

There will be an optional review session on Sunday, 12/16 in Keyes 105 at 4 PM.

There will also be office hours from 1-2pm Monday, 12/10 through Friday, 12/14.  On Monday and Tuesday Prof. Madison will be in the Chem Help Center (Keyes 104). On Wednesday through Friday, come to her office (Keyes 314).

Practice exams are posted on our web page.  The Final Exam Equation Sheet is available as well.


Week 14 Schedule: Section B

In our last week of classes we will be building on our understanding of intermolecular forces to investigate why solutions have the properties that they do.  Why are some solids insoluble while others readily dissolve? Why do cold beverages stay carbonated better than warm ones?  How can we use properties of solutions to make frozen ice cream?

Homework #12 is due on Wednesday.  Additional practice problems will be posted on Mastering Chemistry to give you a chance to practice the material covered in chapter 13.

Monday Lecture Material: Lecture Slides 12-3Class notes 12-3

Wednesday Lecture Material: Lecture Slides 12-5class notes 12-5

Friday Lecture Material: Lecture Slides 12-7class notes 12-7

Additional Resources: The downside to salting our roads

Week 14 Sat 12/2, Sun 12/3 Mon 12/3 Tue 12/4 Wed 12/5 Thu 12/6 Fri 12/7
In Class Chapter 13 Chapter 13 Chapter 13 and Chapter 12
Learning Objectives Relate intermolecular forces to properties of solutions Do calculations related to colligative properties. Describe structures of solids and relate their structures to the properties
Topic Properties of Solutions Properties of Solutions Applications and Modern Materials
Outside of Class
Homework Work on HW #12 Finish HW#12 Homework #12 is due at 11:59pm
Reading 1st Read of Chapter 13 2nd Read of Chapter 13
Other Things to Remember Office Hours 2:30-4:00 Office Hours 1:00-2:30
Practice Problems 13.2, 13.7, 13.15, 13.17, 13.29, 13.27 13.39, 13.51, 13.61, 13.63, 13.69, 13.75 13.85

Making White Light – materials research for a better world

Incandescent bulbs are one of the most energy-inefficient products in daily use,” Joanna McKittrick says. Touch a regular old 100-W light bulb after it’s been lit for a few minutes, and you’ll see what she means.

Less than 5% of the electrical energy that goes into the tungsten filament inside is converted to visible light, explains McKittrick, a luminescent materials specialist at the University of California, San Diego. The rest is wasted as heat that, should you follow our instructions, will burn your fingers.

Incandescents “basically haven’t changed since Thomas Edison invented them” about 140 years ago, she says.

Discovered via computational screening for new phosphors, this compound (above) is the first member of the previously unknown Sr-Li-Al-O crystal family. Black outline = unit cell. Gold = Sr. Red = Li. Green = Al. Blue = O.

Bulbs that contain light-emitting diodes (LEDs), on the other hand, can produce the same amount of white light but barely feel warm to the touch. That’s because LEDs are more energy efficient. A 15-to-20-W LED can produce the same brightness as a 100-W incandescent, roughly 1,500 lumens. LEDs are also less fragile and can last tens of thousands of hours longer. Nevertheless, these modern alternatives currently account for less than 10% of lighting worldwide, according to data from the U.S. Department of Energy.

more …

Week 13 Schedule: Section B

This week we will build off of the concepts of molecular structure, polarity,  and dipole moments to understand how intermolecular forces stick molecules to each other in the liquid and solid phases.  We will explain properties of liquids and solids as well as their phase changes from the intermolecular forces that occur between molecules.

Reminder: Exam #3 is on Wednesday.  More information can be found here.  There is a review session on Monday at 7pm.

Homework #12 will be due next week on Wed. December 5th.

Monday Lecture Materials: Lecture slides 11-26Class notes 11-26

Wednesday Lecture Materials: Lecture slides 11-28Lecture slides 11-28-With soln to PracticeClass notes 11-28

Viscosity and the Pitch Drop Experiment

Friday Lecture Materials: Lecture Slides 11-30

Surface Tension in Space:

Week 13 Mon 11/26 Tue 11/27 Wed 11/28 Thu 11/29 Fri 11/30
In Class Chapter 11 Chapter 11 Chapter 11
Learning Objectives Molecular Comparison of solids, liquids and gases. Relating molecular structure to intermolecular forces. Relating properties of liquids to their intermolecular forces. Structures and bonding of solids.
Topic Liquids and Intermolecular Forces Liquids and Intermolecular Forces Liquids and Intermolecular Forces
Outside of Class
Homework Work on Homework #12
Reading 1st read of chapter 11 2nd read of chapter 11
Other Things to Remember Review Session 5pm-7pm Keyes 105 3rd Exam is Tonight from 5-7pm in Keyes 105 Office hours 1:00-2:30pm
Practice Problems 11.12, 11.15, 11.17, 11.21, 11.22 11.29, 11.32, 11.37, 11.39, 11.45 11.51, 11.55, 11.59, 11.61, 11.71

Solids and Liquids – Making the Oceanographer Happy

Reading chapters 11 and 13

Intermolecular Forces:
London, dipole-dipole, hydrogen bonding, ion-dipole
Comparison of forces
Properties of  Solids, Liquids, and Gases
Phase changes
Heating curves

Resources:   hydrogen boding in biological structures,  Chapter 11 Images 2018, Chapter 11 Notes, Chapter 13 Slides 2018, Chapter 13 notes




Third Exam and Review Session

Reminder: Exam 3 is Wednesday, Nov. 28.  Exam Locations: Keyes 105, 102, 103, and 114.

Practice exams and their solutions can be found on the Sample Exam page.  The relevant files are Practice Exam 3, Exam 3 (with answers) from 2016, and Practice Exam 3 2017.  You are strongly encouraged to do these practice exams before Monday 11/26.  

Exam information: Exam 3 will be held on Wed, Nov. 28 from 5:00-7:00 pm. You may work for the entire 2 hours, but the exam is expected to take most students 60 min. The exam will cover the class material from chapters 1-10 and laboratory material from up to and including experiment 9.  Chapters 6-9 will be emphasized (Electronic Structure of Atoms through Molecular Geometries and Bonding Theories).   Allowed exam items are pens/pencils and a course-approved calculator. You will be provided with a periodic table and equation sheet.

There will be an optional review session on Monday, 11/26 in Keyes 105 at 7 PM.

Equation Sheet Exam 3

“Week” 12: Section B

On Monday we will look at more challenging and integrative practice problems from chapter 9.  These practice problems will help you prepare for exam #3 which will take place on Wednesday, Nov 28th at 5pm.

Be sure to look at the practice exams posted under “Sample Exams and Exam Solutions” over the next week.  I also recommend that you do the practice problems posted on this blog as well as those posted on Mastering Chemistry.

I hope you have a fantastic and restful Thanksgiving!

Monday Lecture Material: Lecture Slides 11-19Class notes and solutions to Integrative Examples 11-19

Week 12 Sat 11/17 Mon 11/19 Tue 11/20 Wed 11/21 Thu 11/22 Fri 11/23
In Class Chapter 9 No Class No Class
Learning Objectives Compare and contrast the 4 bonding theories. Apply the 4 bonding theories to challenging molecules.
Topic Bonding Theories
Outside of Class
Homework Work on HW #11 Work on HW #11 Finish HW #11 Homework #11 is due at 11:59pm
Reading Read chapter 9 First read of Chapter 11
Tasks Eat & Relax Attempt Practice Exam #3
Practice Problems 9.85, 9.89, 9.91, 9.97, 9.99

Play with this! Geometry Builder


Week 11: Section B

This week we will continue our discussion of molecular bonding.  We will learn how to turn our two dimensional Lewis structures into to three dimensional molecular geometries.  By the end of the week we will be able to apply and analyze four theories of molecular bonding: Valence Shell Electron Pair Repulsion theory, Valence Bond theory, Hybrid Orbitals, and Molecular Orbital Theory.

Homework #10 is posted on Mastering Chemistry and it covers chapter 8. It is due on Wednesday at midnight.

Monday Lecture Material:Lecture Slides 11-12class notes 11-12

Wednesday Lecture Material: Lecture Slides 11-14class notes 11-14

Friday Lecture Material:Lecture Slides 11-16class notes 11-16

Week 11 Sat, Sun 11/10-11 Mon 11/12 Tue 11/13 Wed 11/14 Thu 11/15 Fri 11/16
In Class Chapter 9 Chapter 9 Chapter 9
Learning Objectives Describe the 3D structure of molecules based on VSEPR theory. Relate the hybrid orbitals used in bonding and to the 3D structure of molecules. Explain how molecular orbital theory is used to describe bonding in diatomic molecules
Topic Bonding Theories: VESPR Bonding Theories: Valence Bond Theory and Hybrid Orbitals Bonding Theories: Molecular Orbital Theory
Activities Balloon Models Building Molecular Models Will liquid O2 stick to a magnetic?
Outside of Class
Homework Work on HW #10 Work on HW #10 Work on HW #10 Homework #10 is due at 11:59pm Start HW #11 Work on HW#11 (Due Tues. 11/20 at Midnight)
Reading 1st Read of Chapter 9 2nd Read of Chapter 9
Other Things to Remember Special Office Hours Sun. 1pm-3pm Office Hours 2:30-4:00 Office Hours 1-2:30
Practice Problems 9.13, 9.17, 9.21, 9.27, 9.37 9.45, 9.49, 9.53. 9.55, 9.61, 9.63 9.59, 9.61, 9.69, 9.71

For your entertainment, a remake of “Shape of You” but with a mash-up of all the 4 bonding theories that we’ll discuss this week.

Week XI – Advanced Bonding – King

Reading:  Chapter 9

Homework:  Please see Mastering Chemistry

 Lecture Outline:

Molecular Shapes and VSEPR
Bond Strength and Energies
Valence Bond Theory
Molecular Orbitals  – Wave Example ISimple Wave II

Resources:  Chapter 9 Slides, Chapter 9 Notes 2018Chemical Education Molecule Viewer

Why we care about the shapes of Molecules –